BIOCHEMICAL TESTS Reducing and non-Reducing Sugars Sugars can be classified as either reducing or non-reducing based on their ability to reduce copper(II) ions to copper (I) ions during the Benedict’s Test. Reducing sugar have contain free aldehyde or ketone group and have the ability to reduce copper(II) ions to copper (I) ions during the Benedict’s Test. All monosaccharides are reducing sugars while only some dissacharides are reducing sugar. Examples of reducing sugar are: Monosaccharides
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The reaction rate can be studied by measuring the time taken for sufficient quantity of yellow sulfur to be formed. Over time‚ a ‘’cross’’ marked on a piece of paper under the conical flask gradually disappears when viewed from above. 1 time taken for the ‘’cross’’ to disappear because the amount of sulfur formed is considered fixed. To study the order of reaction‚ the experiment is repeated by varying the concentration of each of the reactants (Na2S2O3
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OxidatiOn and ReductiOn OxidatiOn & ReductiOn 9.2 9 Introduction to oxidation and reduction Redox equations Some common oxidising agents and reducing agents (EXT) 9.3 Reactivity 9.4 Voltaic cells 19.1 Standard electrode potentials (AHL) 9.5 Electrolytic cells 19.2 cORe 9.1 Electrolysis (AHL) TOK Are oxidation numbers real? I remember contemplating on the nature of reality back in Chapters 2 and 4‚ with regard to electrons and hybridization respectively
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William son Eth er Synth esis Introduction In this reaction‚ an alcohol is deprotonated to form a good nucleophile‚ which then attacks the electrophile methyl iodide to form an ether. Tetrabutylammonium bromide‚ a phase transfer catalyst‚ is used to carry ions back and forth between the organic phase and the aqueous phase. OH O NaOH + NaI + H2O CH3I Before coming to lab‚ please review the following techniques: "Reluxing a reaction‚" "Extraction and washing‚" "Drying an Organic Solvent‚" "Evaporating
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though there is no visible reaction initially. Shortly thereafter‚ the liquid suddenly turns to a shade of dark blue. This clock reaction uses ammonium persulfate to oxidize iodide ions to iodine. 2I- (aq) + S2O82- (aq) → I2 (aq) + 2SO42- (aq) Subsequently‚ sodium thiosulfate is used to reduce iodine back to iodide before the iodine can complex with the starch to form the characteristic blue-black color. I2 (aq) + 2S2O32- (aq) → 2I- (aq) + S4O62- (aq) An important factor that affects
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produce iodide ion (I-) and dehydroascorbic acid‚ as shown in the following equation: [IMAGE] + I2(aq) -----------> + 2H+(aq) + 2I-(aq) Ascorbic acid (Vit. C) Dehydroascorbic acid However‚ since iodine is only slightly soluble in water‚ ascorgic acid should not be titrated directly by a standard iodine solution‚ since the end point of titration is not o obvious. Instead‚ back titration will be employed. The titration of a reducing agent with iodine to produce iodide ion is
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Transition Metals 1a) The d-orbitals of a free transition metal atom or ion are degenerate (all have the same energy.) However‚ when transition metals form coordination complexes‚ the d-orbitals of the metal interact with the electron cloud of the ligands in such a manner that the d-orbitals become non-degenerate (not all having the same energy.) The way in which the orbitals are split into different energy levels is dependent on the geometry of the complex. Crystal field theory can be used to predict
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Antioxidant Concept: Vitamin C (ascorbic acid) is an antioxidant. The amount of vitamin C content in food can be found out by titrating with an oxidising agent‚ e.g. iodine. In the reaction‚ vitamin C is oxidised‚ while iodine is reduced to iodide ions. The endpoint is determined by the formation of blue-black starch-iodine complex when all vitamin C is oxidised and excess iodine is free to react with the starch solution added as indicator. Introduction Vitamin C is an important component of
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Add a 2.0 gram iron rod to the solution and observe the reaction. 2 Fe + 3 CuSO4 = 3 Cu + Fe2(SO4)3 The new product is iron (III) sulfate‚ it contains the Fe 3+ ion which is brown. Lead (II) nitrate and potassium iodide solutions Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. Pb(NO3)2 + 2 KI = 2 KNO3 + PbI2 2. Magnesium metal and hydrochloric acid solution Place
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(KMnO4) and oxalate ion (C2O42-) C. Iodine clock reaction A. REACTION BETWEEN LEAD NITRATE AND POTASSIUM CHROMATE SOLUTIONS Lead nitrate reacts with potassium chromate to form yellow lead chromate precipitate and aqueous potassium nitrate. The formation of a yellow precipitate indicates the completion of the reaction. The reaction is extremely fast. Pb(NO3)2 (aq) + K2CrO4 (aq) → PbCrO4 (s) + KNO3 (aq) B. REACTION BETWEEN POTASSIUM PERMANGANATE AND OXALATE ION The reaction between
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